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Ionic Compounds: Naming

Ionic Compounds: Naming. Naming Binary Ionic Compounds. Always name the metal (the cation/+ ion) first 2. Write stem of nonmetal (the anion/ - ion) 3. Add the ending “ide” to the nonmetal. Nitr. Ox. Fluor. Phosph. Sulf. Chlor. Arsen. Selen. Brom. Tellur. Iod.

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Ionic Compounds: Naming

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  1. Ionic Compounds: Naming

  2. Naming Binary Ionic Compounds • Always name the metal (the cation/+ ion) first 2. Write stem of nonmetal (the anion/ - ion) 3. Add the ending “ide” to the nonmetal

  3. Nitr Ox Fluor Phosph Sulf Chlor Arsen Selen Brom Tellur Iod Hydr is the stem for H Stems of nonmetals

  4. The First Step in Naming • Find the metal on the PT • If the metal has only one oxidation state it’s easy • If the metal has more than one oxidation state, there’s an extra step

  5. Metals with one oxidation state • CaO • BaS • AlN • LiCl • Al2Se3 • Na2O • K3N • MgF2 Calcium Oxide Barium Sulfide Aluminum Nitride Lithium Chloride Aluminum Selenide Sodium Oxide Potassium Nitride Magnesium Fluoride

  6. Metals with > 1 oxidation state • Use the formula to figure out which oxidation state the metal ion has • Ex: Fe can be Fe+2or Fe+3 • Name FeO and Fe2O3 • two different compounds • cannot name both iron oxide • every formula has 1 name only

  7. FeO and Fe2O3 • Compounds are electrically neutral • Oxygen is -2 1 O which is -2 FeO so Fe must be +2 Name: Iron (II) oxide (roman numeral II = charge on Fe)

  8. Each Fe is +3 Iron (III) oxide FeO and Fe2O3 • Compounds are electrically neutral • Oxygen is -2 Each O is -2 Fe2O3 There are 3 O’s 3 X (-2) = -6 Total negative charge Total positive charge must be +6

  9. Name the followingHint: Positive Always First Titanium (III) chloride • TiCl3 • Mn2O4 • Co2O3 • PdBr2 • AuCl3 • MoN • MnO • TiO Manganese (IV) oxide Cobalt (III) oxide Palladium (II) bromide Gold (III) chloride Molybdenum (III) nitride Manganese (II) oxide Titanium (II) oxide

  10. SO42- CO32- PO43- OH- POLYATOMIC IONS • group of covalently bonded atoms that have a charge • Table E: (+)’ve or (–)’ve • polyatomic ions have “names” • polyatomic ions can form ionic bonds with oppositely-charged ions

  11. Ternary Compounds • contain 3 or more elements • usually contain a polyatomic ion • if polyatomic is (+) it’s bonded to a nonmetal • if polyatomic is (–) it’s bonded to a metal • sometimes 2 polyatomics are bonded together

  12. Formulas with polyatomics • What’s the formula for the compound formed from NH4+1 and Cl-1? • The charges must add up to zero, so just write the symbols, positive first! NH4Cl

  13. Try a few more: NaOH • Na+ and OH- • K + and HCO3-1 • Mg+2 and CO3-2 • Li + and NO3- • NH4+ and CN- • Ca+2 and SO4-2 KHCO3 MgCO3 LiNO3 NH4CN CaSO4

  14. These are more challenging: Mg3(PO4)2 • Mg+2 and (PO4)-3 • (NH4)+1 and S-2 • Al+3 and (NO3)-1 • Fe+2 and OH-1 • Hg2+2 and SCN-1 • Mg+2 and HCO3- • Al+3 and C2O42- (NH4)2S Al(NO3)3 Fe(OH)2 Hg2(SCN)2 Mg(HCO3)2 Al2(C2O4)3

  15. Be(ClO3)2 Some of the most challenging are Zn(NO3)2 • Zinc + Nitrate ion • Magnesium + Hydroxide ion • Lithium + Carbonate ion • Ammonium ion + Bromine • Potassium + Sulfate ion • Calcium + Phosphate ion • Beryllium + Chlorate ion • Ammonium ion + Sulfate ion Mg(OH)2 Li2CO3 NH4Br K2SO4 Ca3(PO4)2 (NH4)2SO4

  16. Naming compounds with polyatomics • polyatomic ions have names (Table E) • naming is parallel to binary naming • positive always written first • if (+)’ve ion is a metal, check to see how many oxidation states it has • if > 1 name must have a roman numeral • if (–)’ve is polyatomic - 2nd part of name is name of polyatomic (don’t modify ending)

  17. Name the following Sodium hydroxide • NaOH • KHCO3 • LiNO3 • CaSO4 • Al(NO3)3 • Fe(OH)2 • CuSO4 • CuSCN Potassium hydrogen carbonate Lithium nitrate Calcium sulfate Aluminum nitrate Iron (II) hydroxide Copper (II) sulfate Copper (I) thiocyanate

  18. Summary for Binary Ionic Compounds • Compounds are electrically neutral • Formula: positive first, always • If metal has more than 1 oxidation state, name has a roman numeral • Name = metal + stem of nonmetal + ide

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